|Publication number||US4081520 A|
|Application number||US 05/770,360|
|Publication date||Mar 28, 1978|
|Filing date||Feb 22, 1977|
|Priority date||Mar 19, 1976|
|Also published as||CA1079931A, CA1079931A1, CA1080433A, CA1080433A1, CA1080434A, CA1080434A1|
|Publication number||05770360, 770360, US 4081520 A, US 4081520A, US-A-4081520, US4081520 A, US4081520A|
|Inventors||Richard Swindells, Maurice C. J. Fredette|
|Original Assignee||Erco Industries Limited|
|Export Citation||BiBTeX, EndNote, RefMan|
|Patent Citations (5), Referenced by (59), Classifications (7), Legal Events (5)|
|External Links: USPTO, USPTO Assignment, Espacenet|
The present invention relates to the production of chlorine dioxide.
It is known from U.S. Pat. No. 2,881,052 to form chlorine dioxide by the reduction of an acid aqueous chlorate solution using methanol. However, the reaction involved is quite slow, requiring a time-consuming operation in a succession of reactors and results in a large volume of liquid effluent containing sulphuric acid, unreacted sodium chlorate and sodium sulphate by-product. The efficiency of conversion of chlorate to chlorine dioxide is quite low, generally not exceeding about 90%. Air typically is passed into the reaction medium to dilute the chlorine dioxide.
The overall reaction involved in this prior art process, known commonly as the "Solvay" process, may be represented by the equation:
2NaClO3 + 2H2 SO4 + CH3 OH→2ClO2 + 2NaHSO4 + HCHO + 2H2 O (1)
It has surprisingly been found that the efficiency of the Solvay process may be substantially improved by using a high total acid normality and carrying out the reaction in a single chambered generator-evaporator-crystallizer vessel, as described in more detail below.
It has been observed that the efficiency of methanol utilization in this invention in the conversion of chlorate to chlorine dioxide often exceeds 100%, indicating that the oxidation products of methanol, namely formaldehyde formic acid also have a role in the efficient production of chlorine dioxide in accordance with this invention. Formaldehyde, formic acid and other organic reducing agents for sodium chlorate may be used in this invention.
In a single chambered generator-evaporator-crystallizer vessel as used in the present invention, chlorine dioxide is generated in continuous manner from a reaction medium which is held in the reaction vessel and is maintained at its boiling point at the prevailing absolute pressure in the reaction vessel and at a temperature below which substantial decomposition of chlorine dioxide occurs. The reaction vessel is maintained under a subatmospheric pressure to maintain the reaction medium at the boiling point and the water evaporated from the reaction medium is used as a diluent gas for the chlorine dioxide. After start-up, by-product acid salt of the cation of the chlorate and the anion of the acid feed is formed, its concentration builds up until the reaction medium is saturated thereby, and the salt deposits from the reaction medium in the reaction vessel once saturation is reached for removal therefrom.
The process is generally conducted under steady state conditions in which the quantity of water introduced to the reaction vessel with the reactants is balanced by the quantity of water removed from the reaction vessel, mainly as diluent gas for the chlorine dioxide, so that the liquid level in the reaction vessel is maintained substantially constant.
In this invention, sodium chlorate, sulphuric acid and methanol are fed to the reaction medium.
The reaction medium has a high acidity. The term "acidity" is usually considered to refer to the total acidity present as determined by titration with a solution of a known concentration of sodium hydroxide to a preselected pH end point. This determination is expressed in terms of normality, i.e., the equivalent number of gram atoms of hydrogen per liter of solution corresponding to the value titrated, and may be referred to as the "total acid normality". The term "total acid normality" is used herein to define acidity in the sense first described.
The reaction medium used in the present invention has a high total acid normality above about 9 normal. In the absence of purposely added chloride ions, it has been found that, with increasing total sulphuric acid normality, the efficiency of conversion of sodium chlorate to chlorine dioxide increases.
Further, it was found that under steady state conditions, varying quantities of sodium chloride were detected in the reaction medium and the quantity of sodium chloride present decreased substantially with increasing total acid normality.
The efficiency of the conversion of sodium chlorate to chlorine dioxide in accordance with reaction (1) above may rise to a very high level, typically up to 99 to 100%, and hence considerably in excess of that achieved in the conventional Solvay process.
The purity of the chlorine dioxide formed, in terms of contamination by chlorine, increases with increasing total acid normality, indicating an increasing tendency for reaction according to equation (1) to occur with increasing total acid normality.
In this invention, the by-product sodium sulphate which is deposited from the reaction medium in the reaction vessel is in the form of sodium bisulphate (NaHSO4), or sodium sesquisulphate (Na3 H(SO4)2).
In order to utilize the acid values of this sodium sulphate, it may be added to the reaction medium of another chlorine dioxide-producing process in which sodium chlorate and sodium chloride and/or hydrogen chloride are reacted in an acid aqueous medium at a total acid normality of less than about 4.8 normal, the sodium acid sulphate being used to provide all or part of the acid requirement of a chlorine dioxide-producing process. Such a tandem chlorine-dioxide generating procedure is described in more detail in U.S. Pat. No. 3,789,108.
Not only is the efficiency of the Solvay process improved by operation in accordance with the present invention, but the necessity to handle liquid overflow containing sulphuric acid, sodium sulphate and some sodium chlorate and the necessity to use external sources of diluent gas when utilizing the conventional Solvay process, are avoided.
The following Example illustrates the invention further.
A chlorine dioxide generator was run under different reaction conditions and in each case the efficiency of production of chlorine dioxide and the purity of the chlorine dioxide were determined. In each case, sodium chlorate solution, sulphuric acid and methanol were the only feeds to the generator, the reaction medium was held at its boiling point under a subatmospheric pressure and sodium acid bisulphate deposited from the reaction medium.
Three separate operations were carried out and the conditions and results are set forth in the following Table:
TABLE__________________________________________________________________________ Run No. 1 2 3__________________________________________________________________________Temperature 64° C 66° C 74° CPressure 114 mm Hg 106 mm Hg 135 mm Hg MeOH 100% 5.1ml/min 33% 3.8 ml/min 33% 3.4ml/min H2 SO4 18M 2.9 ml/min 9M 7.0 ml/min 9M 3.6 ml/min NaClO3 1.8M 19.1ml/min 1.8M 38.7ml/min 6.74M 10.5ml/minGenerator liquor: H2 SO4 4.40N 8.04N 9.3N NaClO3 1.56M 0.87M 1.1M NaCl* 0.39M 0.04M 0.003MCrystal 60% Na2 SO4 40% Na3 H(SO4)2 Na3 H(SO4)2 NaHSO4Chlorine dioxide 0.21g/l/min 0.36g/l/min 0.48g/l/minproductionGas analysis 84% ClO2 16% Cl2 88% ClO2 12% Cl2 99% ClO2 <1%Cl2Efficiency based 87.7% 78% >99%on chlorateEfficiency based 14% 87% 127%on MeOHFeed requirements 1.72 0.28 0.19 lb.CH3 OH/lb.ClO2 produced__________________________________________________________________________ Note: *No sodium chloride was purposely added initially, although the sodium chlorate feed contains about 0.003 lb of NaCl impurity per lb/ of NaClO3.
It will be seen from the results of the above Table that as the total acid normality of the reaction medium increases, the rate of production of chlorine dioxide increases, the purity of the chlorine dioxide increases, the quantity of sodium chloride present in the reaction medium decreases and the efficiency of production of chlorine dioxide in terms of chlorate consumed increases.
A typical Solvay process for producing chlorine dioxide has an efficiency in terms of conversion of chlorate to chlorine dioxide of about 89% with a methanol requirement of 0.20 lbs. CH3 OH per lb. ClO2 produced. It will be seen from the above results that by operating under the conditions of run No. 3, i.e., at an acid normality above about 9 normal, a substantial increase in efficiency can be effected.
The present invention, therefore, provides considerable improvements over the prior art Solvay process for producing chlorine dioxide. Modifications are possible within the scope of the invention.
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|U.S. Classification||423/478, 423/511, 423/551, 423/520|
|Mar 4, 1985||AS||Assignment|
Owner name: TENNECO CANADA INC.
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